The number of manganeses ions in tetrahedral and octahedral sites respectively in `Mn_3O_4` are

Options

A. one `Mn^(2+) and " two"Mn^(3+)` ions
B. one `Mn^(3+) and " two"Mn^(2+)` ions
C. two `Mn^(3+) and " two"Mn^(2+)` ions
D. two `Mn^(2+) and " two"Mn^(3+)` ions

Answer

To determine the number of manganese ions in tetrahedral and octahedral sites in the compound \( \text{Mn}_3\text{O}_4 \), we can follow these steps:

### Step 1: Understand the Structure of \( \text{Mn}_3\text{O}_4 \)
- \( \text{Mn}_3\text{O}_4 \) is a mixed oxide, often referred to as a spinel structure. Spinels can generally be represented as \( \text{AB}_2\text{O}_4 \), where A and B are metals in different oxidation states.

### Step 2: Identify the Oxidation States
- In \( \text{Mn}_3\text{O}_4 \), manganese exists in two oxidation states: \( \text{Mn}^{2+} \) and \( \text{Mn}^{3+} \).
- The formula indicates that there are three manganese ions in total.

### Step 3: Determine the Distribution of Manganese Ions
- In a normal spinel structure, the \( \text{Mn}^{2+} \) ions occupy tetrahedral sites, while the \( \text{Mn}^{3+} \) ions occupy octahedral sites.
- For \( \text{Mn}_3\text{O}_4 \):
- There is 1 \( \text{Mn}^{2+} \) ion in the tetrahedral site.
- There are 2 \( \text{Mn}^{3+} \) ions in the octahedral sites.

### Step 4: Conclusion
- Therefore, the number of manganese ions in tetrahedral and octahedral sites respectively in \( \text{Mn}_3\text{O}_4 \) is:
- Tetrahedral sites: 1 \( \text{Mn}^{2+} \)
- Octahedral sites: 2 \( \text{Mn}^{3+} \)

### Final Answer
The number of manganese ions in tetrahedral and octahedral sites in \( \text{Mn}_3\text{O}_4 \) are 1 and 2, respectively.

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